T tx3 New Member 10+ Year Member Joined Jun 20, 2009 Messages 6 Reaction score 0 Points 0 Pre-Dental Sep 5, 2009 #1 Advertisement - Members don't see this ad What is the pH of a solution with 0.5 mol of carbonic acid and 1.0 mol of bicarbonate dissolved in 2L? If anyone could help me get started on this problem I would really appreciate it. The textbook explanation confuses me. Thank you!
Advertisement - Members don't see this ad What is the pH of a solution with 0.5 mol of carbonic acid and 1.0 mol of bicarbonate dissolved in 2L? If anyone could help me get started on this problem I would really appreciate it. The textbook explanation confuses me. Thank you!
hausee Full Member 10+ Year Member 15+ Year Member Joined Nov 20, 2006 Messages 595 Reaction score 0 Points 0 Location UCSD Sep 5, 2009 #2 Do you have a pka of carbonic acid? If you do you can use pka to figure out H+ concentration because bicarbonate concentration already given. Upvote 0 Downvote
Do you have a pka of carbonic acid? If you do you can use pka to figure out H+ concentration because bicarbonate concentration already given.
M mehron Full Member 10+ Year Member Joined Jul 26, 2009 Messages 17 Reaction score 0 Points 0 Pre-Dental Sep 5, 2009 #3 Here's how I would do it: H2CO3 + H2O <--> HCO3- + H+ I 0.25M 0.5M 0 C -x +x +x E 0.25-x 0.5+x x PKa pf H2CO3= (x+0.5)(x)/(0.25-x) Find x pH= -log [x] Upvote 0 Downvote
Here's how I would do it: H2CO3 + H2O <--> HCO3- + H+ I 0.25M 0.5M 0 C -x +x +x E 0.25-x 0.5+x x PKa pf H2CO3= (x+0.5)(x)/(0.25-x) Find x pH= -log [x]
T tx3 New Member 10+ Year Member Joined Jun 20, 2009 Messages 6 Reaction score 0 Points 0 Pre-Dental Sep 5, 2009 #4 pka = 10.24 Last edited: Sep 5, 2009 Upvote 0 Downvote
T tx3 New Member 10+ Year Member Joined Jun 20, 2009 Messages 6 Reaction score 0 Points 0 Pre-Dental Sep 5, 2009 #5 thank you for your help Upvote 0 Downvote
Z zellyen Full Member 10+ Year Member Joined Jul 21, 2009 Messages 310 Reaction score 0 Points 0 Sep 5, 2009 #6 PKa pf H2CO3= (x+0.5)(x)/(0.25-x) dont you mean Ka or am i missing something 😵 Upvote 0 Downvote
